### Electrochemical Reactions Worksheet**Instructions:**- Please provide balanced equations for the reactions described below.- Ensure each equation is balanced in terms of mass and charge.---**1. Write a balanced equation for the half-reaction that happens at the cathode.**| Reaction | ||----------|----------|| | |---**2. Write a balanced equation for the half-reaction that happens at the anode.**| Reaction | ||----------|----------|| | |---**3. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**| Reaction | ||----------|----------|| | | --- *Note:* Each equation should include the appropriate states of matter (solid, liquid, aqueous, gas) and ensure the correct stoichiometric coefficients are used to balance the equation.---This worksheet is designed to aid in understanding and practicing the balancing of electrochemical reactions, including both half-reactions at the cathode and anode, and the overall spontaneous reaction that occurs in an electrochemical cell. ### Galvanic Cell DesignA chemist designs a galvanic cell that uses these two half-reactions:| half-reaction | standard reduction potential || -------------------------------------------- | ------------------------------------ || \( 2 \text{IO}_3^- (aq) + 12 \text{H}^+ (aq) + 10 e^- \rightarrow \text{I}_2 (s) + 6 \text{H}_2 \text{O} (l) \) | \( E^0_{\text{red}} = +1.195 \, \text{V} \) || \( \text{Cl}_2 (g) + 2 e^- \rightarrow 2 \text{Cl}^- (aq) \) | \( E^0_{\text{red}} = +1.359 \, \text{V} \) |This table outlines the half-reactions along with their standard reduction potentials (\( E^0_{\text{red}} \)) in volts. In a galvanic cell, these potentials help determine which reactions will occur at the anode and cathode, thus pointing to the overall cell potential.

Two half cell reactions of a galvanic cell are given.

Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How many Faraday is needed to deposit 5 moles of Aluminium (Al) from AlCl3 solution using electrolysis process?
How many Faraday is needed to deposit 1.4 g of Aluminium (Al) from AlCl3 solution using electrolysis process.
Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 中 Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 G
Explain the working of a Fuel cell and list the different types of Fuel cells with brief explanation of each type.
5. Explain what is meant by a fuel cell. Provide a balanced equation to represent the reaction in any fuel cell of your choice.
When creating an electrochemical cell, why is it important to prevent the reactants from any direct contact?
Explain the working of the oxygen probe by referring to reactions that take place at the cathodeand anode
In 200 to 250 words Describe what would happen if pure platinum plates were used for the electrodes instead of copper and silver plates in an electrolysis apparatus.
Write the half-reaction that occurs at the anode during the electrolysis of NaCl. Include physical states and use single arrow in your equation. Incorrect. Recall that reduction takes place at the cathode, so the substance must be gaining electrons. Write the half-reaction that occurs at the cathode during the electrolysis of NaCl. Include physical states and use single arrow in your equation. Incorrect. Is your reaction balanced? There should be no electrons in a balanced final equation. Write the overall cell reaction for the electrolysis of NaCl. Include physical states and use single arrow in your equation.
What is the general layout/structures of the anode and cathode?
Which cell is generally used in hearing aids?Name the material of the anode,cathode and the electrolyte. Write the reactions involved.
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential Exed half-reaction 2 H2O(1)+2e → H2(g)+2OH (aq) Ε red -0.83 V 2+ Zn(aq)+2e →>> Zn(s) E = = -0.763 V 'red Answer the following questions about this cell.